For the equation
`N_(2)O_(5)(g)=2NO_(2)(g)+(1//2)O_(2)(g)`, calculate the mole fraction of `N_(2)O_(5)(g)` decomposed at a constant volume and temperature, if the initial pressure is `600 mm Hg` and the pressure at any time is `960 mm Hg`. Assume ideal gas behaviour.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Understand the Reaction
The reaction given is:
\[ N_2O_5(g) \rightarrow 2NO_2(g) + \frac{1}{2}O_2(g) \]

### Step 2: Define Initial and Final Pressures
- Initial pressure of \( N_2O_5 \) = \( P_i = 600 \, \text{mm Hg} \)
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